How does water overcome the attractive forces holding a solute particle in a solid?
A)
by surrounding the solute particles
B)
by isolating the solvent particles
C)
by interspersing with the solvent molecules
D)
by surrounding the solvent particles
2.
What does the expression “like dissolves like” mean?
A)
In general, polar compounds will dissolve in a polar solvent.
B)
In general, polar solutes will not dissolve in a polar solvent.
C)
In general, non-polar compounds will dissolve in a polar solvent.
D)
In general, polar compounds will dissolve in a non-polar solvent like water.
3.
What affects the rate at which solutes dissolve?
A)
temperature of the solution
B)
surface area of the solute
C)
concentration of the solute
D)
all of the above
4.
Of the following, which could be electrolytes?
A)
PCl3
B)
CaCl2
C)
both of the above
D)
neither of the above
5.
Which of the following are not electrolytes?
A)
NaI
B)
CaCl2
C)
KBr
D)
NO2
6.
According to the solubility table, KBr should be what?
A)
soluble
B)
insoluble
C)
molecular
D)
sparingly soluble
7.
What kind of compound is AgCl in water?
A)
insoluble
B)
soluble
C)
dissolvable
D)
not enough information to tell
8.
In the reaction Cu + 2 HCl ® CuCl2 + H2, what has happened to the acid?
A)
The Cu has been reduced.
B)
The Cl– has been oxidized.
C)
The H+ has been reduced.
D)
Nothing has happened.
9.
The addition of KOH to HCl is what kind of reaction?
A)
a reduction–oxidation that does not make a precipitate
B)
a reduction–oxidation that makes a precipitate
C)
a neutralization that makes salt and water
D)
an addition that makes salt and water
10.
The pH of a solution with a [H+] = 1.0 ´ 10–8 is what?
A)
4
B)
8
C)
12
D)
can't be determined
11.
What is a solution with a pH of 12?
A)
neutral
B)
acidic
C)
basic
D)
concentrated
12.
Attractive forces that exist between particles are called what?
A)
intermolecular forces
B)
intramolecular forces
C)
heteromolecular forces
D)
intravenous-molecular forces
13.
To what is the positive region of a polar molecule attracted?
A)
a magnet
B)
the positive region of a neighboring molecule
C)
the negative region of a neighboring molecule
D)
to a non-polar molecule, thus inducing a dipole
14.
Which of the following will form hydrogen bonds?
A)
methanol, CH3OH
B)
water, H2O
C)
neither of the above
D)
both of the above
15.
If the reaction AgNO3 + NaCl ® NaNO3 + AgCl were written out as a total ionic reaction, which ions would be the spectator ions?
A)
Ag+ and NO3–
B)
Na+ and Ag+
C)
Na+ and NO3–
D)
Cl– and NO3–
16.
At the boiling point of a liquid, what two forces are equal?
A)
vapor density and internal pressure
B)
vapor density and external pressure
C)
vapor pressure and external temperature
D)
vapor pressure and external pressure
17.
What is the boiling point of a solution made from 1.10 g KCN in 750 g of water? (Kbp = 0.512oC/m)
18.
What is the molarity of a solution made from 0.25 mol of KBr and 0.80 L of water?
19.
What is the one factor upon which boiling point elevation depends?
20.
predict the products and write a balanced net ionic equation.
a. sodium phosphate reacts with zinc bromide
b. potassium chloride reacts with silver sulfate
21.
If 300 mL of a solution with a 1.5 M is diluted to 750 mL, what is its new molarity?
22.
What do all weak acids have in common?
23.
What is the name of the following acidic compound, HI?
24.
What is occurring at the freezing point of a liquid?
25.
What is a weak electrolyte?
26.
What is the freezing point of a water solution made from 12.9 g NaCl and 400 g of water?(Kfp = -1.86oC/m)
27.
What is the molality of a solution made from 13.4 g of NaCl in 250 g of water?
28.
What is the molarity of a solution made from 65.0 g of Na2SO4 and 2.30 L of water?
29.
Assuming a similar molality, which of the three compounds—Na2S, NaCl, or Al2(SO4)3— should have the highest freezing point (closest to 0) and which should have the lowest freezing point?
30.
How are London dispersion forces characterized?
Chapters 7 and 8
1.
What do all alkenes have in common?
A)
at least one double bond
B)
at least one triple bond
C)
at least one carbon–carbon bond
D)
carbon–hydrogen bonds
2.
Compounds with a triple bond, alkynes, all share a general molecular formula. What is it?
A)
CnH2n-4
B)
CnH2n+2
C)
CnH2n
D)
CnH2n-2
3.
What is the first rule of naming branched isomers?
A)
count the number of methyl branches
B)
find the longest branch
C)
find the number of branches
D)
find the longest continuous carbon chain
4.
What is the geometry of the very simple molecule carbon monoxide?
A)
linear
B)
bent, planar
C)
square planar
D)
horizontal
5.
Cylohexane has what molecular formula?
A)
C6H14
B)
C6H12
C)
C6H16
D)
C6H13
6.
What is the name of the following compound?
A)
cyclopentane
B)
cyclobutane
C)
cyclohexane
D)
cyclooctane
7.
What is the proper line structure for cyclooctane?
A)
.
B)
.
C)
.
D)
.
8.
What is the name of a cyclohexane molecule when one of the carbon atoms in the ring also has a –CH3 attached to it?
A)
cycloheptane
B)
methylcyclohexane
C)
methylcycloheptane
D)
cyclohexane
9.
What shape does the methane molecule, CH4, have?
A)
bent
B)
a square pyramid
C)
planar
D)
a tetrahedral
10.
What do the valence shells of all the noble gas elements have in common?
A)
a large size for its row on the periodic table
B)
a high ability to lose electrons
C)
a filled electron shell
D)
a high affinity for further electrons
11.
What is the shape of the water molecule?
A)
trigonal planar
B)
linear
C)
bent
D)
trigonal pyramidal
12.
What is the octet rule?
A)
Elements form bonds to become isoelectronic with the noble gases.
B)
Elements form bonds to avoid becoming isoelectronic with the noble gases.
C)
Elements do not form bonds to become isoelectronic with the noble gases.
D)
Elements do not form bonds to avoid becoming isoelectronic with the noble gases.
13.
The correct Lewis dot structure for potassium is what?
A)
.K.
B)
.K
C)
.Pt
D)
.Pt.
14.
What is the correct Lewis dot structure for Se?
A)
:Se:
B)
C)
D)
15.
Lewis structures with single lines indicate what kind of bonding?
A)
covalent, two-electron bonding
B)
ionic, two-electron bonding
C)
covalent, four-electron bonding
D)
ionic, four-electron bonding
16.
What is the correct Lewis structure for ethyne, C2H2, also known by the common name acetylene?
A)
H—H–C–C
B)
H–C—C–H
C)
H–C=C–H
D)
H–CºC–H
17.
What does the double line, which looks much like an equals sign, represent in Lewis structures?
A)
A 2-electron single bond
B)
A 4-electron double bond
C)
A 2-electron double bond
D)
A 4-electron single bond
18.
What does valence shell electron pair repulsion theory help determine?
A)
atomic geometry
B)
molecular geometry
C)
molecular size
D)
atomic size
19.
What does the term “functional group” refer to in organic chemistry?
20.
What is the general molecular formula of a cyclic alkane?
21.
Draw and name the isomers of heptane
22.
What is wrong with the statement, “nonpolar molecules must always be composed of nonpolar bonds?”
23.
The term “valence shell electron pair repulsion” indicates that electron pairs do what when they are close to each other?
24.
What does the term “resonance structure” mean?
25.
Draw the Lewis structure, name the VSEPR structure, and indicate if polar or nonpolar
Compound Lewis Structure VSEPR Polarity
a. PH3
b. SO2
c. CBr3H
d. PO4 3-
e. C2H2
Chapters 9 and 10
1.
What ingredients are needed for a fire?
1.
What ingredients are needed for a fire?
A)
a fuel source
B)
oxygen gas
C)
heat
D)
all of the above
2.
Which is the balanced equation for the complete combustion of methanol (CH3OH) in oxygen gas?
A)
2 CH3OH + O2 ® 2 CO2 + 4 H2O
B)
2 CH3OH + 3 O2 ® 2 CO2 + 4 H2O
C)
CH3OH + 3 O2 ® 2 CO2 + 2 H2O
D)
CH3OH + 3 O2 ® CO2 + 4 H2O
3.
What is the oxidation number of chlorine in MgCl2?
A)
–2
B)
–1
C)
0
D)
+1
4.
What is the oxidation number of oxygen in the reactants of the following reaction:
CH4 + 2 O2 ® CO2 + 2 H2O?
A)
–1
B)
–2
C)
2
D)
0
5.
To what does the term oxidation refer?
A)
the gain of electrons
B)
the movement of electrons
C)
the loss of electrons
D)
the reduction of electrons
6.
What do all exothermic reactions produce?
A)
heat
B)
light
C)
smoke
D)
fumes
7.
When a 500.0 g sample of silica glass changes temperature from 23.0oC to 50.0oC, what amount of heat is involved?
(specific heat capacity for silica glass is 0.75 J/goC)
8.
What is the mass of a piece of aluminum that starts at 100oC, is immersed in a calorimeter with 200 g of water at 25.0oC, and causes the water to rise to a temperature of 29.5oC?(specific heat capacity for aluminum is 0.9J/goC and the specific heat capacity for water is 4.18 J/goC
9.
When gases react according to a balanced chemical equation, such as 2H2(g) + O2 (g) ® 2 H2O(g), what do the coefficients represent?
A)
the gas masses that react
B)
the gas pressures that react
C)
the gas volumes that react
D)
none of the above
10.
What is the new pressure when a 10-L container of gas at 3,500 mmHg is compressed down to 2.5 L?
11.
When the temperature of a gas rises by a factor of 3, what should happen to the pressure of the gas, all other factors being constant?
A)
It should rise by a factor of 3.
B)
It should decrease by a factor of 3.
C)
The pressure should remain unchanged.
D)
not enough information to tell
12.
When the volume of a gas decreases by 1/2, what happens to its temperature if all other factors remain unchanged?
13.
How many liters of a gas are equal to one mole of the gas at STP?
14.
5.00 L of chlorine gas is at 15oC. What temperature will the gas have when the volume changes to
12.5 L?
15.
If a gas at 15 atm occupying 5.0 L at 25oC is pressurized to 25 atm at 10 L, what will the new temperature of the gas be?
16.
Identify what is reduced and what is oxidized in the ractions below.
a. Br2 + K2O ® O2 + KBr
b. Zn + Cl2 ® ZnCl2
17.
Write and balance the equation for the combustion of the following:
a. C2H5OH
b. nonane
c. C8H16O
18.
If 2.5 g of Ne and some Ar are mixed in a 3 L clylinder at 15oC, the pressure gauge reads 798 kPa. What is the pressure exerted by each gas and what amount in grams do you have of Ar?
19.
list and define the 3 types of chromatography.
20.
Find the amount in grams of 6.5L of Kr at STP. What is STP?
chapters 5 and 6
a. sodium phosphate reacts with zinc bromide
b. potassium chloride reacts with silver sulfate
Chapters 7 and 8
.
.
.
.
Compound Lewis Structure VSEPR Polarity
a. PH3
b. SO2
c. CBr3H
d. PO4 3-
e. C2H2
Chapters 9 and 10
2.
CH4 + 2 O2 ® CO2 + 2 H2O?
(specific heat capacity for silica glass is 0.75 J/goC)
12.5 L?
a. Br2 + K2O ® O2 + KBr
b. Zn + Cl2 ® ZnCl2
a. C2H5OH
b. nonane
c. C8H16O
||